The reaction of nitrogen gas and oxygen gas to form nitrogen monoxide gas is shown below. If the measured concentrations of all three chemicals at some point in time are: [N2] = 0.80 M

[O2] = 0.050 M
[NO] = 0.10 M
Which statement is TRUE about the reaction at this point in time? N2(g) + O2(g) ⇄ 2 NO(g) K = 0.10

1. The reaction is at equilibrium.
2. The reverse reaction is occurring at a faster rate than the forward reaction.
3. The forward reaction is occurring at a faster rate than the reverse reaction.
4. This set of concentration values is impossible because the concentrations of N2 and O2 must be the same.

Two nitro no2 groups are chemically bonded to a patch of surface. they can't move to another location on the surface, but they can rotate (see sketch at right). it turns out that the amount of rotational kinetic energy each no2 group can have is required to be a multiple of ε, where =ε×1.010−24 j. in other words, each no2 group could have ε of rotational kinetic energy, or 2ε, or 3ε, and so forth — but it cannot have just any old amount of rotational kinetic energy. suppose the total rotational kinetic energy in this system is initially known to be 32ε. then, some heat is removed from the system, and the total rotational kinetic energy falls to 18ε. calculate the change in entropy. round your answer to 3 significant digits, and be sure it has the correct unit symbol.

11) burning your hand when accidentally touching a hot plate is an example of which heat transfer? a. conduction b. convection c. radiation d. none of these

The empirical formula of a compound is ch2o and its mass is 120 amu/molecule, what is its formula?